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Solvated electron

January 01, 1970

A solvated electron is a free electron in a solution, in which it behaves like an anion.[1] An electron's being solvated in a solution means it is bound by the solution.[2] The notation for a solvated electron in formulas of chemical reactions is "e−". Often, discussions of solvated electrons focus on their solutions in ammonia, which are stable for days, but solvated electrons also occur in water and many other solvents – in fact, in any solvent that mediates outer-sphere electron transfer. The solvated electron is responsible for a great deal of radiation chemistry.

Ammonia solutions edit

Liquid ammonia will dissolve all of the alkali metals and other electropositive metals such as Ca,[3] Sr, Ba, Eu, and Yb (also Mg using an electrolytic process[4]), giving characteristic blue solutions. For alkali metals in liquid ammonia, the solution is blue when dilute and copper-colored when more concentrated (> 3 molar).[5] These solutions conduct electricity. The blue colour of the solution is due to ammoniated electrons, which absorb energy in the visible region of light. The diffusivity of the solvated electron in liquid ammonia can be determined using potential-step chronoamperometry.[6]

Solvated electrons in ammonia are the anions of salts called electrides.

Na + 6 NH3 → [Na(NH3)6]+ + e−

The reaction is reversible: evaporation of the ammonia solution produces a film of metallic sodium.

Case study: Li in NH3 edit

 
Solutions obtained by dissolution of lithium in liquid ammonia. The solution at the top has a dark blue color and the lower one a golden color. The colors are characteristic of solvated electrons at electronically insulating and metallic concentrations, respectively.

A lithium–ammonia solution at −60 °C is saturated at about 15 mol% metal (MPM). When the concentration is increased in this range electrical conductivity increases from 10−2 to 104 Ω−1cm−1 (larger than liquid mercury). At around 8 MPM, a "transition to the metallic state" (TMS) takes place (also called a "metal-to-nonmetal transition" (MNMT)). At 4 MPM a liquid-liquid phase separation takes place: the less dense gold-colored phase becomes immiscible from a denser blue phase. Above 8 MPM the solution is bronze/gold-colored. In the same concentration range the overall density decreases by 30%.

Other solvents edit

Alkali metals also dissolve in some small primary amines, such as methylamine and ethylamine[7] and hexamethylphosphoramide, forming blue solutions. THF dissolves alkali metal, but a Birch reduction (see § Applications) analogue does not proceed without a diamine ligand.[8] Solvated electron solutions of the alkaline earth metals magnesium, calcium, strontium and barium in ethylenediamine have been used to intercalate graphite with these metals.[9]

Water edit

Solvated electrons are involved in the reaction of alkali metals with water, even though the solvated electron has only a fleeting existence.[10] Below pH = 9.6 the hydrated electron reacts with the hydronium ion giving atomic hydrogen, which in turn can react with the hydrated electron giving hydroxide ion and usual molecular hydrogen H2.[11]

Solvated electrons can be found even in the gas phase. This implies their possible existence in the upper atmosphere of Earth and involvement in nucleation and aerosol formation.[12]

Its standard electrode potential value is -2.77 V.[13] The equivalent conductivity of 177 Mho cm2 is similar to that of hydroxide ion. This value of equivalent conductivity corresponds to a diffusivity of 4.75   cm2s−1.[14]

Reactivity edit

Although quite stable, the blue ammonia solutions containing solvated electrons degrade rapidly in the presence of catalysts to give colorless solutions of sodium amide:

2 [Na(NH3)6]+e− → H2 + 2 NaNH2 + 10 NH3

Electride salts can be isolated by the addition of macrocyclic ligands such as crown ether and cryptands to solutions containing solvated electrons. These ligands strongly bind the cations and prevent their re-reduction by the electron.

[Na(NH3)6]+e− + cryptand → [Na(cryptand)]+e−+ 6 NH3

The solvated electron reacts with oxygen to form a superoxide radical (O2.−).[15] With nitrous oxide, solvated electrons react to form hydroxyl radicals (HO.).[16]

Applications edit

Solvated electrons are involved in electrode processes, a broad area with many technical applications (electrosynthesis, electroplating, electrowinning).

A specialized use of sodium-ammonia solutions is the Birch reduction. Other reactions where sodium is used as a reducing agent also are assumed to involve solvated electrons, e.g. the use of sodium in ethanol as in the Bouveault–Blanc reduction.

Work by Cullen et al. showed that metal-ammonia solutions can be used to intercalate a range of layered materials, which can then be exfoliated in polar, aprotic solvents, to produce ionic solutions of two-dimensional materials.[17] An example of this is the intercalation of graphite with potassium and ammonia, which is then exfoliated by spontaneous dissolution in THF to produce a graphenide solution. [18]

History edit

The observation of the color of metal-electride solutions is generally attributed to Humphry Davy. In 1807–1809, he examined the addition of grains of potassium to gaseous ammonia (liquefaction of ammonia was invented in 1823).[19] James Ballantyne Hannay and J. Hogarth repeated the experiments with sodium in 1879–1880.[20] W. Weyl in 1864 and C. A. Seely in 1871 used liquid ammonia, whereas Hamilton Cady in 1897 related the ionizing properties of ammonia to that of water.[21][22][23] Charles A. Kraus measured the electrical conductance of metal ammonia solutions and in 1907 attributed it to the electrons liberated from the metal.[24][25] In 1918, G. E. Gibson and W. L. Argo introduced the solvated electron concept.[26] They noted based on absorption spectra that different metals and different solvents (methylamine, ethylamine) produce the same blue color, attributed to a common species, the solvated electron. In the 1970s, solid salts containing electrons as the anion were characterized.[27]

References edit

  1. ^ Dye, J. L. (2003). "Electrons as Anions". Science. 301 (5633): 607–608. doi:10.1126/science.1088103. PMID 12893933. S2CID 93768664.
  2. ^ Schindewolf, U. (1968). "Formation and Properties of Solvated Electrons". Angewandte Chemie International Edition in English. 7 (3): 190–203. doi:10.1002/anie.196801901.
  3. ^ Edwin M. Kaiser (2001). "Calcium–Ammonia". Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.rc003. ISBN 978-0471936237.
  4. ^ Combellas, C; Kanoufi, F; Thiébault, A (2001). "Solutions of solvated electrons in liquid ammonia". Journal of Electroanalytical Chemistry. 499: 144–151. doi:10.1016/S0022-0728(00)00504-0.
  5. ^ Cotton, F. A.; Wilkinson, G. (1972). Advanced Inorganic Chemistry. John Wiley and Sons Inc. ISBN 978-0-471-17560-5.
  6. ^ Harima, Yutaka; Aoyagui, Shigeru (1980). "The diffusion coefficient of solvated electrons in liquid ammonia". Journal of Electroanalytical Chemistry and Interfacial Electrochemistry. 109 (1–3): 167–177. doi:10.1016/S0022-0728(80)80115-X.
  7. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  8. ^ Burrows, James; Kamo, Shogo; Koide, Kazunori (2021-11-05). "Scalable Birch reduction with lithium and ethylenediamine in tetrahydrofuran". Science. 374 (6568): 741–746. doi:10.1126/science.abk3099. ISSN 0036-8075. PMID 34735232. S2CID 243761715.
  9. ^ Xu, Wei; Lerner, Michael M. (2018). "A New and Facile Route Using Electride Solutions to Intercalate Alkaline Earth Ions into Graphite". Chemistry of Materials. 30 (19): 6930–6935. doi:10.1021/acs.chemmater.8b03421. S2CID 105295721.
  10. ^ Walker, D.C. (1966). "Production of hydrated electron". Canadian Journal of Chemistry. 44 (18): 2226–. doi:10.1139/v66-336.
  11. ^ Jortner, Joshua; Noyes, Richard M. (1966). "Some Thermodynamic Properties of the Hydrated Electron". The Journal of Physical Chemistry. 70 (3): 770–774. doi:10.1021/j100875a026.
  12. ^ Arnold, F. (1981). "Solvated electrons in the upper atmosphere". Nature. 294 (5843): 732–733. doi:10.1038/294732a0. S2CID 4364255.
  13. ^ Baxendale, J. H. (1964). "Effects of Oxygen and pH in the Radiation Chemistry of Aqueous Solutions". Radiation Research Supplement. 4: 114–138. doi:10.2307/3583572. JSTOR 3583572.
  14. ^ Hart, Edwin J. (1969). "The Hydrated Electron". Survey of Progress in Chemistry. 5: 129–184. doi:10.1016/B978-0-12-395706-1.50010-8. ISBN 9780123957061. S2CID 94713398.
  15. ^ Hayyan, Maan; Hashim, Mohd Ali; Alnashef, Inas M. (2016). "Superoxide Ion: Generation and Chemical Implications". Chemical Reviews. 116 (5): 3029–3085. doi:10.1021/acs.chemrev.5b00407. PMID 26875845.
  16. ^ Janata, Eberhard; Schuler, Robert H. (1982). "Rate constant for scavenging eaq- in nitrous oxide-saturated solutions". The Journal of Physical Chemistry. 86 (11): 2078–2084. doi:10.1021/j100208a035.
  17. ^ Cullen, Patrick L.; Cox, Kathleen M.; Bin Subhan, Mohammed K.; Picco, Loren; Payton, Oliver D.; Buckley, David J.; Miller, Thomas S.; Hodge, Stephen A.; Skipper, Neal T.; Tileli, Vasiliki; Howard, Christopher A. (March 2017). "Ionic solutions of two-dimensional materials". Nature Chemistry. 9 (3): 244–249. doi:10.1038/nchem.2650. hdl:1983/360e652b-ca32-444d-b880-63aeac05f6ac. ISSN 1755-4349. PMID 28221358.
  18. ^ Angel, Gyen Ming A.; Mansor, Noramalina; Jervis, Rhodri; Rana, Zahra; Gibbs, Chris; Seel, Andrew; Kilpatrick, Alexander F. R.; Shearing, Paul R.; Howard, Christopher A.; Brett, Dan J. L.; Cullen, Patrick L. (6 August 2020). "Realising the electrochemical stability of graphene: scalable synthesis of an ultra-durable platinum catalyst for the oxygen reduction reaction". Nanoscale. 12 (30): 16113–16122. doi:10.1039/D0NR03326J. ISSN 2040-3372. PMID 32699875.
  19. ^ Thomas, Sir John Meurig; Edwards, Peter; Kuznetsov, Vladimir L. (January 2008). "Sir Humphry Davy: Boundless Chemist, Physicist, Poet and Man of Action". ChemPhysChem. 9 (1): 59–66. doi:10.1002/cphc.200700686. PMID 18175370. An entry from Humphry Davy′s laboratory notebook of November 1808. It reads "When 8 Grains of potassium were heated in ammoniacal gas—it assumed a beautiful metallic appearance & gradually became of a fine blue colour".
  20. ^ Hannay, J. B.; Hogarth, James (26 February 1880). "On the solubility of solids in gases". Proceedings of the Royal Society of London. 30 (201): 178–188.
  21. ^ Weyl, W. (1864). "Ueber Metallammonium-Verbindungen" [On metal-ammonium compounds]. Annalen der Physik und Chemie (in German). 121: 601–612.
    • See also: Weyl, W. (1864). "Ueber die Bildung des Ammoniums und einiger Ammonium-Metalle" [On the formation of ammonium and of some ammonium metals]. Annalen der Physik und Chemie (in German). 123: 350–367.
  22. ^ Seely, Charles A. (14 April 1871). "On ammonium and the solubility of metals without chemical action". The Chemical News. 23 (594): 169–170.
  23. ^ Cady, Hamilton P. (1897). "The electrolysis and electrolytic conductivity of certain substances dissolved in liquid ammonia". The Journal of Physical Chemistry. 1 (11): 707–713. doi:10.1021/j150593a001.
  24. ^ Kraus, Charles A. (1907). "Solutions of metals in non-metallic solvents; I. General properties of solutions of metals in liquid ammonia". J. Am. Chem. Soc. 29 (11): 1557–1571. doi:10.1021/ja01965a003.
  25. ^ Zurek, Eva (2009). "A molecular perspective on lithium–ammonia solutions". Angew. Chem. Int. Ed. 48 (44): 8198–8232. doi:10.1002/anie.200900373. PMID 19821473.
  26. ^ Gibson, G. E.; Argo, W. L. (1918). "The absorption spectra of the blue solutions of certain alkali and alkaline earth metals in liquid ammonia and methylamine". J. Am. Chem. Soc. 40 (9): 1327–1361. doi:10.1021/ja02242a003.
  27. ^ Dye, J. L. (2003). "Electrons as anions". Science. 301 (5633): 607–608. doi:10.1126/science.1088103. PMID 12893933. S2CID 93768664.

Further reading edit

  • Sagar, D. M.; Colin; Bain, D.; Verlet, Jan R. R. (2010). "Hydrated Electrons at the Water/Air Interface". J. Am. Chem. Soc. 132 (20): 6917–6919. doi:10.1021/ja101176r. PMID 20433171. S2CID 207049708.
  • Martyna, Glenn (1993). "Electronic states in metal-ammonia solutions". Physical Review Letters. 71 (2): 267–270. Bibcode:1993PhRvL..71..267D. doi:10.1103/physrevlett.71.267. PMID 10054906.
  • Martyna, Glenn (1993). "Quantum simulation studies of singlet and triplet bipolarons in liquid ammonia". Journal of Chemical Physics. 98 (1): 555–563. Bibcode:1993JChPh..98..555M. doi:10.1063/1.464650.
  • Solvated Electron. Advances in Chemistry. Vol. 50. 1965. doi:10.1021/ba-1965-0050. ISBN 978-0-8412-0051-7.
  • Anbar, Michael (1965). "Reactions of the Hydrated Electron". Solvated Electron. Advances in Chemistry. Vol. 50. pp. 55–81. doi:10.1021/ba-1965-0050.ch006. ISBN 978-0-8412-0051-7.
  • Abel, B.; Buck, U.; Sobolewski, A. L.; Domcke, W. (2012). "On the nature and signatures of the solvated electron in water". Phys. Chem. Chem. Phys. 14 (1): 22–34. Bibcode:2012PCCP...14...22A. doi:10.1039/C1CP21803D. PMID 22075842.
  • Harima, Y.; Aoyagui, S. (1981). "Determination of the chemical solvation energy of the solvated electron". Journal of Electroanalytical Chemistry and Interfacial Electrochemistry. 129 (1–2): 349–352. doi:10.1016/S0022-0728(81)80027-7.
  • Hart, Edwin J. (1969). "The Hydrated Electron". Survey of Progress in Chemistry Volume 5. Survey of Progress in Chemistry. Vol. 5. pp. 129–184. doi:10.1016/B978-0-12-395706-1.50010-8. ISBN 9780123957061. S2CID 94713398.
  • The electrochemistry of the solvated electron. Technische Universiteit Eindhoven.
  • IAEA On the Electrolytic Generation of Hydrated Electron.
  • Fundamentals of Radiation Chemistry, chapter 6, p. 145–198, Academic Press, 1999.
  • Tables of bimolecular rate constants of hydrated electrons, hydrogen atoms and hydroxyl radicals with inorganic and organic compounds, International Journal of Applied Radiation and Isotopes Anbar, Neta

January 01, 1970
solvated, electron, solvated, electron, free, electron, solution, which, behaves, like, anion, electron, being, solvated, solution, means, bound, solution, notation, solvated, electron, formulas, chemical, reactions, often, discussions, solvated, electrons, fo. A solvated electron is a free electron in a solution in which it behaves like an anion 1 An electron s being solvated in a solution means it is bound by the solution 2 The notation for a solvated electron in formulas of chemical reactions is e Often discussions of solvated electrons focus on their solutions in ammonia which are stable for days but solvated electrons also occur in water and many other solvents in fact in any solvent that mediates outer sphere electron transfer The solvated electron is responsible for a great deal of radiation chemistry Contents 1 Ammonia solutions 1 1 Case study Li in NH3 2 Other solvents 3 Water 4 Reactivity 5 Applications 6 History 7 References 8 Further readingAmmonia solutions editLiquid ammonia will dissolve all of the alkali metals and other electropositive metals such as Ca 3 Sr Ba Eu and Yb also Mg using an electrolytic process 4 giving characteristic blue solutions For alkali metals in liquid ammonia the solution is blue when dilute and copper colored when more concentrated gt 3 molar 5 These solutions conduct electricity The blue colour of the solution is due to ammoniated electrons which absorb energy in the visible region of light The diffusivity of the solvated electron in liquid ammonia can be determined using potential step chronoamperometry 6 Solvated electrons in ammonia are the anions of salts called electrides Na 6 NH3 Na NH3 6 e The reaction is reversible evaporation of the ammonia solution produces a film of metallic sodium Case study Li in NH3 edit nbsp Solutions obtained by dissolution of lithium in liquid ammonia The solution at the top has a dark blue color and the lower one a golden color The colors are characteristic of solvated electrons at electronically insulating and metallic concentrations respectively A lithium ammonia solution at 60 C is saturated at about 15 mol metal MPM When the concentration is increased in this range electrical conductivity increases from 10 2 to 104 W 1cm 1 larger than liquid mercury At around 8 MPM a transition to the metallic state TMS takes place also called a metal to nonmetal transition MNMT At 4 MPM a liquid liquid phase separation takes place the less dense gold colored phase becomes immiscible from a denser blue phase Above 8 MPM the solution is bronze gold colored In the same concentration range the overall density decreases by 30 Other solvents editAlkali metals also dissolve in some small primary amines such as methylamine and ethylamine 7 and hexamethylphosphoramide forming blue solutions THF dissolves alkali metal but a Birch reduction see Applications analogue does not proceed without a diamine ligand 8 Solvated electron solutions of the alkaline earth metals magnesium calcium strontium and barium in ethylenediamine have been used to intercalate graphite with these metals 9 Water editSolvated electrons are involved in the reaction of alkali metals with water even though the solvated electron has only a fleeting existence 10 Below pH 9 6 the hydrated electron reacts with the hydronium ion giving atomic hydrogen which in turn can react with the hydrated electron giving hydroxide ion and usual molecular hydrogen H2 11 Solvated electrons can be found even in the gas phase This implies their possible existence in the upper atmosphere of Earth and involvement in nucleation and aerosol formation 12 Its standard electrode potential value is 2 77 V 13 The equivalent conductivity of 177 Mho cm2 is similar to that of hydroxide ion This value of equivalent conductivity corresponds to a diffusivity of 4 75 10 5 displaystyle times 10 5 nbsp cm2s 1 14 Reactivity editAlthough quite stable the blue ammonia solutions containing solvated electrons degrade rapidly in the presence of catalysts to give colorless solutions of sodium amide 2 Na NH3 6 e H2 2 NaNH2 10 NH3 Electride salts can be isolated by the addition of macrocyclic ligands such as crown ether and cryptands to solutions containing solvated electrons These ligands strongly bind the cations and prevent their re reduction by the electron Na NH3 6 e cryptand Na cryptand e 6 NH3 The solvated electron reacts with oxygen to form a superoxide radical O2 15 With nitrous oxide solvated electrons react to form hydroxyl radicals HO 16 Applications editSolvated electrons are involved in electrode processes a broad area with many technical applications electrosynthesis electroplating electrowinning A specialized use of sodium ammonia solutions is the Birch reduction Other reactions where sodium is used as a reducing agent also are assumed to involve solvated electrons e g the use of sodium in ethanol as in the Bouveault Blanc reduction Work by Cullen et al showed that metal ammonia solutions can be used to intercalate a range of layered materials which can then be exfoliated in polar aprotic solvents to produce ionic solutions of two dimensional materials 17 An example of this is the intercalation of graphite with potassium and ammonia which is then exfoliated by spontaneous dissolution in THF to produce a graphenide solution 18 History editThe observation of the color of metal electride solutions is generally attributed to Humphry Davy In 1807 1809 he examined the addition of grains of potassium to gaseous ammonia liquefaction of ammonia was invented in 1823 19 James Ballantyne Hannay and J Hogarth repeated the experiments with sodium in 1879 1880 20 W Weyl in 1864 and C A Seely in 1871 used liquid ammonia whereas Hamilton Cady in 1897 related the ionizing properties of ammonia to that of water 21 22 23 Charles A Kraus measured the electrical conductance of metal ammonia solutions and in 1907 attributed it to the electrons liberated from the metal 24 25 In 1918 G E Gibson and W L Argo introduced the solvated electron concept 26 They noted based on absorption spectra that different metals and different solvents methylamine ethylamine produce the same blue color attributed to a common species the solvated electron In the 1970s solid salts containing electrons as the anion were characterized 27 References edit Dye J L 2003 Electrons as Anions Science 301 5633 607 608 doi 10 1126 science 1088103 PMID 12893933 S2CID 93768664 Schindewolf U 1968 Formation and Properties of Solvated Electrons Angewandte Chemie International Edition in English 7 3 190 203 doi 10 1002 anie 196801901 Edwin M Kaiser 2001 Calcium Ammonia Encyclopedia of Reagents for Organic Synthesis doi 10 1002 047084289X rc003 ISBN 978 0471936237 Combellas C Kanoufi F Thiebault A 2001 Solutions of solvated electrons in liquid ammonia Journal of Electroanalytical Chemistry 499 144 151 doi 10 1016 S0022 0728 00 00504 0 Cotton F A Wilkinson G 1972 Advanced Inorganic Chemistry John Wiley and Sons Inc ISBN 978 0 471 17560 5 Harima Yutaka Aoyagui Shigeru 1980 The diffusion coefficient of solvated electrons in liquid ammonia Journal of Electroanalytical Chemistry and Interfacial Electrochemistry 109 1 3 167 177 doi 10 1016 S0022 0728 80 80115 X Greenwood Norman N Earnshaw Alan 1997 Chemistry of the Elements 2nd ed Butterworth Heinemann ISBN 978 0 08 037941 8 Burrows James Kamo Shogo Koide Kazunori 2021 11 05 Scalable Birch reduction with lithium and ethylenediamine in tetrahydrofuran Science 374 6568 741 746 doi 10 1126 science abk3099 ISSN 0036 8075 PMID 34735232 S2CID 243761715 Xu Wei Lerner Michael M 2018 A New and Facile Route Using Electride Solutions to Intercalate Alkaline Earth Ions into Graphite Chemistry of Materials 30 19 6930 6935 doi 10 1021 acs chemmater 8b03421 S2CID 105295721 Walker D C 1966 Production of hydrated electron Canadian Journal of Chemistry 44 18 2226 doi 10 1139 v66 336 Jortner Joshua Noyes Richard M 1966 Some Thermodynamic Properties of the Hydrated Electron The Journal of Physical Chemistry 70 3 770 774 doi 10 1021 j100875a026 Arnold F 1981 Solvated electrons in the upper atmosphere Nature 294 5843 732 733 doi 10 1038 294732a0 S2CID 4364255 Baxendale J H 1964 Effects of Oxygen and pH in the Radiation Chemistry of Aqueous Solutions Radiation Research Supplement 4 114 138 doi 10 2307 3583572 JSTOR 3583572 Hart Edwin J 1969 The Hydrated Electron Survey of Progress in Chemistry 5 129 184 doi 10 1016 B978 0 12 395706 1 50010 8 ISBN 9780123957061 S2CID 94713398 Hayyan Maan Hashim Mohd Ali Alnashef Inas M 2016 Superoxide Ion Generation and Chemical Implications Chemical Reviews 116 5 3029 3085 doi 10 1021 acs chemrev 5b00407 PMID 26875845 Janata Eberhard Schuler Robert H 1982 Rate constant for scavenging eaq in nitrous oxide saturated solutions The Journal of Physical Chemistry 86 11 2078 2084 doi 10 1021 j100208a035 Cullen Patrick L Cox Kathleen M Bin Subhan Mohammed K Picco Loren Payton Oliver D Buckley David J Miller Thomas S Hodge Stephen A Skipper Neal T Tileli Vasiliki Howard Christopher A March 2017 Ionic solutions of two dimensional materials Nature Chemistry 9 3 244 249 doi 10 1038 nchem 2650 hdl 1983 360e652b ca32 444d b880 63aeac05f6ac ISSN 1755 4349 PMID 28221358 Angel Gyen Ming A Mansor Noramalina Jervis Rhodri Rana Zahra Gibbs Chris Seel Andrew Kilpatrick Alexander F R Shearing Paul R Howard Christopher A Brett Dan J L Cullen Patrick L 6 August 2020 Realising the electrochemical stability of graphene scalable synthesis of an ultra durable platinum catalyst for the oxygen reduction reaction Nanoscale 12 30 16113 16122 doi 10 1039 D0NR03326J ISSN 2040 3372 PMID 32699875 Thomas Sir John Meurig Edwards Peter Kuznetsov Vladimir L January 2008 Sir Humphry Davy Boundless Chemist Physicist Poet and Man of Action ChemPhysChem 9 1 59 66 doi 10 1002 cphc 200700686 PMID 18175370 An entry from Humphry Davy s laboratory notebook of November 1808 It reads When 8 Grains of potassium were heated in ammoniacal gas it assumed a beautiful metallic appearance amp gradually became of a fine blue colour Hannay J B Hogarth James 26 February 1880 On the solubility of solids in gases Proceedings of the Royal Society of London 30 201 178 188 Weyl W 1864 Ueber Metallammonium Verbindungen On metal ammonium compounds Annalen der Physik und Chemie in German 121 601 612 See also Weyl W 1864 Ueber die Bildung des Ammoniums und einiger Ammonium Metalle On the formation of ammonium and of some ammonium metals Annalen der Physik und Chemie in German 123 350 367 Seely Charles A 14 April 1871 On ammonium and the solubility of metals without chemical action The Chemical News 23 594 169 170 Cady Hamilton P 1897 The electrolysis and electrolytic conductivity of certain substances dissolved in liquid ammonia The Journal of Physical Chemistry 1 11 707 713 doi 10 1021 j150593a001 Kraus Charles A 1907 Solutions of metals in non metallic solvents I General properties of solutions of metals in liquid ammonia J Am Chem Soc 29 11 1557 1571 doi 10 1021 ja01965a003 Zurek Eva 2009 A molecular perspective on lithium ammonia solutions Angew Chem Int Ed 48 44 8198 8232 doi 10 1002 anie 200900373 PMID 19821473 Gibson G E Argo W L 1918 The absorption spectra of the blue solutions of certain alkali and alkaline earth metals in liquid ammonia and methylamine J Am Chem Soc 40 9 1327 1361 doi 10 1021 ja02242a003 Dye J L 2003 Electrons as anions Science 301 5633 607 608 doi 10 1126 science 1088103 PMID 12893933 S2CID 93768664 Further reading editSagar D M Colin Bain D Verlet Jan R R 2010 Hydrated Electrons at the Water Air Interface J Am Chem Soc 132 20 6917 6919 doi 10 1021 ja101176r PMID 20433171 S2CID 207049708 Martyna Glenn 1993 Electronic states in metal ammonia solutions Physical Review Letters 71 2 267 270 Bibcode 1993PhRvL 71 267D doi 10 1103 physrevlett 71 267 PMID 10054906 Martyna Glenn 1993 Quantum simulation studies of singlet and triplet bipolarons in liquid ammonia Journal of Chemical Physics 98 1 555 563 Bibcode 1993JChPh 98 555M doi 10 1063 1 464650 Solvated Electron Advances in Chemistry Vol 50 1965 doi 10 1021 ba 1965 0050 ISBN 978 0 8412 0051 7 Anbar Michael 1965 Reactions of the Hydrated Electron Solvated Electron Advances in Chemistry Vol 50 pp 55 81 doi 10 1021 ba 1965 0050 ch006 ISBN 978 0 8412 0051 7 Abel B Buck U Sobolewski A L Domcke W 2012 On the nature and signatures of the solvated electron in water Phys Chem Chem Phys 14 1 22 34 Bibcode 2012PCCP 14 22A doi 10 1039 C1CP21803D PMID 22075842 Harima Y Aoyagui S 1981 Determination of the chemical solvation energy of the solvated electron Journal of Electroanalytical Chemistry and Interfacial Electrochemistry 129 1 2 349 352 doi 10 1016 S0022 0728 81 80027 7 Hart Edwin J 1969 The Hydrated Electron Survey of Progress in Chemistry Volume 5 Survey of Progress in Chemistry Vol 5 pp 129 184 doi 10 1016 B978 0 12 395706 1 50010 8 ISBN 9780123957061 S2CID 94713398 The electrochemistry of the solvated electron Technische Universiteit Eindhoven IAEA On the Electrolytic Generation of Hydrated Electron Fundamentals of Radiation Chemistry chapter 6 p 145 198 Academic Press 1999 Tables of bimolecular rate constants of hydrated electrons hydrogen atoms and hydroxyl radicals with inorganic and organic compounds International Journal of Applied Radiation and Isotopes Anbar Neta Retrieved from https en wikipedia org w index php title Solvated electron amp oldid 1193880042, wikipedia, wiki, book, books, library,

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